4.6 Excess, Limiting Amounts, Percentage Yield, and Impurities 1

LIMITING and EXCESS REACTANTS Suppose you have a job in a sandwich shop One very popular sandwich has ingredients as follows: 2 slices of bread + 3 slices of meat + 1 slice of cheese

LIMITING and EXCESS REACTANTS 2 slices of bread 3 slices of meat 1 sandwich 1 slice of cheese

LIMITING and EXCESS REACTANTS 2 slices of bread 3 slices of meat 1 sandwich 1 slice of cheese You come to work one day and find the following ingredients:

LIMITING and EXCESS REACTANTS 8 slices of bread 9 slices of meat 1 slice of cheese

NOW, ANSWER THE QUESTIONS ON THE WORKSHEET! 8 slices of bread 9 slices of meat 5 slice of cheese

Most probably you found out: The meat was a limiting ingredient! When you run out of meat, you couldn’t make any more sandwiches even though you had bread and cheese in excess (too much or extra)

Most probably you found out: Molecules react with each other in very similar way!

Each N2 needs 3 H2 molecules to form 2 NH3 N2(g) + 3H2(g) 2NH3(g) Consider the following container of N2 and H2 : How many N2 are there? 5 How many H2 are there? 15 What will this container look like if the reaction between N2 and H2 proceeds to completion? REMEMBER: Each N2 needs 3 H2 molecules to form 2 NH3

This ratio EXACTLY matches the numbers in the balanced equation N2(g) + 3H2(g) 2NH3(g) This ratio EXACTLY matches the numbers in the balanced equation

N2(g) + 3H2(g) 2NH3(g) NOTHING is limiting (too little) and NOTHING is in excess (too much or extra)

Now, consider a different container of N2 and H2: N2(g) + 3H2(g) 2NH3(g) Now, consider a different container of N2 and H2: How many N2 are there? 5 How many H2 are there? 9 What will this container look like if the reaction between N2 and H2 proceeds to completion? REMEMBER: Each N2 needs 3 H2 molecules to form 2 NH3

N2(g) + 3H2(g) 2NH3(g) HYDROGEN is limiting (too little) because it is used up BEFORE all NITROGEN molecules are used.

N2(g) + 3H2(g) 2NH3(g) HYDROGEN limits the amount of AMMONIA (NH3) that can be produced = H2 is a LIMITING REACTANT

N2(g) + 3H2(g) 2NH3(g) NITROGEN is in excess (too much or extra) because the reaction runs out of HYDROGEN molecules first

NITROGEN is called the EXCESS REACTANT N2(g) + 3H2(g) 2NH3(g) NITROGEN is called the EXCESS REACTANT

N2(g) + 3H2(g) 2NH3(g) In real life problems, we MUST know how much PRODUCT is produced. And because this is limited by the LIMITING REACTANT, we must look for a reactant that is LIMITING.

N2(g) + 3H2(g) 2NH3(g) In real life, we don’t count the molecules to find out what are LIMITING and what are EXCESS REACTANTS!

We MUST count by weighing or by calculating the number of moles! N2(g) + 3H2(g) 2NH3(g) We MUST count by weighing or by calculating the number of moles!

SAS Curriculum Pathways Username: alexanderacademy Pick “Vlab: Limiting Reactants”

SAS Curriculum Pathways Answers for Data & Observations: On a separate piece of paper You will have a data table handout as well Answers for Analysis & Conclusions: On a separate piece of paper

Calculating Limiting Reactant! If a sample containing 18.1 g of NH3 is reacted with 90.4 g of CuO, which is the limiting reactant? Which is the excess reactant? How many grams of N2 will be produced? 2NH3(g) + 3CuO(s) N2(g) + 3Cu(s) + 3H2O(g) Calculating Limiting Reactant!

1. USING EACH REACTANT, CALCULATE THE MASS OF N2! If a sample containing 18.1 g of NH3 is reacted with 90.4 g of CuO, which is the limiting reactant? Which is the excess reactant? How many grams of N2 will be produced? 2NH3(g) + 3CuO(s) N2(g) + 3Cu(s) + 3H2O(g) 1. USING EACH REACTANT, CALCULATE THE MASS OF N2! 2. WHICHEVER REACTANT PRODUCES THE SMALLEST AMOUNT OF N2, THAT IS THE LIMITING REACTANT! 3. USE THE NUMBER OF MOLES OF THE LIMITING REACTANT TO CALCULATE THE MASS OF N2.

1. USING EACH REACTANT, CALCULATE THE MASS OF N2! If a sample containing 18.1 g of NH3 is reacted with 90.4 g of CuO, which is the limiting reactant? Which is the excess reactant? How many grams of N2 will be produced? 2NH3(g) + 3CuO(s) N2(g) + 3Cu(s) + 3H2O(g) 1. USING EACH REACTANT, CALCULATE THE MASS OF N2!

2NH3(g) + 3CuO(s) N2(g) + 3Cu(s) + 3H2O(g) If a sample containing 18.1 g of NH3 is reacted with 90.4 g of CuO, which is the limiting reactant? Which is the excess reactant? How many grams of N2 will be produced? 2NH3(g) + 3CuO(s) N2(g) + 3Cu(s) + 3H2O(g) 2. WHICHEVER REACTANT PRODUCES THE SMALLEST AMOUNT OF N2, THAT IS THE LIMITING REACTANT!

2NH3(g) + 3CuO(s) N2(g) + 3Cu(s) + 3H2O(g) If a sample containing 18.1 g of NH3 is reacted with 90.4 g of CuO, which is the limiting reactant? Which is the excess reactant? How many grams of N2 will be produced? 2NH3(g) + 3CuO(s) N2(g) + 3Cu(s) + 3H2O(g) 3. USE THE NUMBER OF MOLES OF THE LIMITING REACTANT TO CALCULATE THE MASS OF N2.

CuO is the Limiting Reactant If a sample containing 18.1 g of NH3 is reacted with 90.4 g of CuO, which is the limiting reactant? Which is the excess reactant? How many grams of N2 will be produced? 2NH3(g) + 3CuO(s) N2(g) + 3Cu(s) + 3H2O(g) 3. USE THE NUMBER OF MOLES OF THE LIMITING REACTANT TO CALCULATE THE MASS OF N2. CuO is the Limiting Reactant

2NH3(g) + 3CuO(s) N2(g) + 3Cu(s) + 3H2O(g) If a sample containing 18.1 g of NH3 is reacted with 90.4g of CuO, which is the limiting reactant? Which is the excess reactant? By how many grams is the NH3 in excess? 2NH3(g) + 3CuO(s) N2(g) + 3Cu(s) + 3H2O(g) 1. Use the mass/moles of THE LIMITING REACTANT to find out the mass of the excess reactant which reacted 2. Take the mass of the excess reactant from the step 1 and subtract it from the original mass of the excess reactant

2NH3(g) + 3CuO(s) N2(g) + 3Cu(s) + 3H2O(g) If a sample containing 18.1 g of NH3 is reacted with 90.4g of CuO, which is the limiting reactant? Which is the excess reactant? By how many grams is the NH3 in excess? 2NH3(g) + 3CuO(s) N2(g) + 3Cu(s) + 3H2O(g) 1. Use the mass/moles of THE LIMITING REACTANT to find out the mass of the excess reactant which reacted

2NH3(g) + 3CuO(s) N2(g) + 3Cu(s) + 3H2O(g) If a sample containing 18.1 g of NH3 is reacted with 90.4g of CuO, which is the limiting reactant? Which is the excess reactant? By how many grams is the NH3 in excess? 2NH3(g) + 3CuO(s) N2(g) + 3Cu(s) + 3H2O(g) 2. Take the mass of the excess reactant from the step 1 and subtract it from the original mass of the excess reactant Mass of the excess reactant which reacted = The original mass of the excess reactant =

Classwork/Homework

PERCENTAGE PURITY 36

PERCENTAGE PURITY It is virtually impossible to obtain a 100% chemical Even chemicals from chemical supply companies include impurities

PERCENTAGE PURITY

PERCENTAGE YIELD 40

PERCENTAGE YIELD WHY DO YOU THINK THIS HAPPENS? Most of the times, the amount of products that we receive from the reaction is less than what we expected based on our calculations and the balanced equation WHY DO YOU THINK THIS HAPPENS? Different reactions happening at the same time (side reactions) Not all of the pure material (product) reacts The products might not be 100% pure Some of the product is lost during the laboratory procedures

THEORETICAL YIELD So, the balanced equation and the stoichiometric calculations will give you ONLY THE EXPECTED (THEORETICAL) YIELD of a product

ACTUAL YIELD THE ACTUAL YIELD When you actually measure (weigh) how much product is produced, this is called: THE ACTUAL YIELD

PERCENTAGE YIELD

2NH3(g) + 3CuO(s) N2(g) + 3Cu(s) + 3H2O(g) If a sample containing 18.1 g of NH3 is reacted with 90.4 g of CuO. How many grams of N2 will be produced? Crisanta did this experiment in a lab, and obtained 9.55 g of N2. What was the percentage yield of the reaction? 2NH3(g) + 3CuO(s) N2(g) + 3Cu(s) + 3H2O(g) Mass of N2 using CuO (limiting reactant): = 90.4 g CuO x 1 mol CuO 79.55g CuO x 1 mol N2 3 mol CuO x 28.0 g N2 1 mol N2 = 10.6 g N2 Theoretical Yield Mass of N2 actually produced in a lab using CuO (limiting reactant): 9.55 g N2 Actual Yield

PERCENTAGE YIELD = 90.1% = 9.55 g N2 10.6 g N2 x 100% Theoretical Yield Actual Yield 9.55 g N2 10.6 g N2 = 90.1% = 9.55 g N2 10.6 g N2 x 100%

HOMEWORK PAGE: 228 PROBLEMS: 4.6 Activity: Charting and Graphing Stoichiometry Practice Problems (do as many as you want/need) The answer key will be given on Monday, after I see 4.6 Activity completed

5 questions – one from each section Chapter 4 TEST Tuesday, May 13th 5 questions – one from each section